A flask that can withstand an internal pressure of 2500 Torr, but no more, is filled with a gas at 21.0 C and 758 Torr and heated. At what temperature will it burst?
To determine the temperature at which the flask will burst, we need to use the gas law equation known as the Ideal Gas Law. The Ideal Gas Law relates the pressure, temperature, and volume of a gas.
The equation is given as:
PV = nRT
Where:
P = pressure (in this case, internal pressure of the flask)
V = volume (not given)
n = number of moles (not given)
R = gas constant (8.314 J/(mol*K))
T = temperature
Since we are only concerned with the temperature at which the flask bursts, we can ignore the volume and moles of gas in this case.
Rearranging the equation, we get:
T = (P * V) / (n * R)
Now, let's substitute the given values into the equation:
P = 2500 Torr (internal pressure of the flask at bursting point)
V = Unknown (volume of the flask, not provided)
n = Unknown (number of moles of gas, not provided)
R = 8.314 J/(mol*K) (gas constant)
To proceed, we need to convert the temperatures to Kelvin, since the gas constant is given in J/(mol*K). The conversion formula is:
T(K) = T(°C) + 273.15
Given:
Initial temperature, T1 = 21.0°C
Final temperature, T2 = Unknown
Converting the initial temperature to Kelvin:
T1(K) = 21.0 + 273.15 = 294.15 K
Now, we can rearrange the equation to solve for the final temperature, T2:
T2 = (P * V) / (n * R)
However, since the volume and number of moles are not provided, we cannot directly compute the final temperature at which the flask will burst. These values are required to accurately solve the equation.
Therefore, without the volume and number of moles of gas, it is not possible to determine the exact temperature at which the flask will burst.